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108 Cards in this Set
- Front
- Back
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Chemistry |
Study of matter and it's properties, composition and changes |
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Matter |
Anything that has mass and occupies space |
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Pure substance |
Matter with uniform composition |
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2 groups of pure substance |
Elements Compounds |
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Elements |
Substance composed of only one kind of atom which cannot be broken down using electricity |
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Compounds |
substance composed of 2 or more kinds of atoms and can be decomposed using heat or electricity |
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Mixtures |
Combinations or pure substances |
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2 groups of mixtures |
Homogeneous Heterogeneous |
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Homogeneous |
Same throughout They are uniform and consist of only one phase |
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Heterogeneous |
Not the same consistrncy throughout May consist of more than one phase |
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Physical change |
Substance maintains chemical properties but changed physically |
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Chemical change |
New substance is formed there is a rearrangement of atoms and/or ions which creates a new compound. Changes are often irreversible |
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Evidence of chemical changes |
Bubbles Color change Formation of precipitate Generation of heat and/or light Odor |
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Who created the periodic table |
Dmitri mendeleyev |
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Atom |
Smallest particle of an element that still represents the chemical properties of the element |
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Nucleus |
Most massive part of the atom. Contains protons and neutrons. Cnetral part of atom |
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Orbits |
Region around and nucleus where electrons found |
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Types of subatomic particles |
Proton Neutron Electron |
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Proton |
Positive charge Mass is 1 |
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Neutron |
No charge Mass is 1 |
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Electrons |
Negative charge Mass of 1/1856 |
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Isotopes |
Same number ifbprotons Different number of neutrons Atomic number is the same but mass number is different |
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Periodic law |
When elements are arranged in order of increasing atomic mass, chemical and physical properties that form patterns and repeat over regular intervals |
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Families |
Vertical columns Similar chemical and physical properties |
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Periods |
Horizontal rows Gradually change from metallic to non metallic from left to right across the row |
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Group names |
Alkali metals Alkaline earth metals Halogens Noble gases Representative elements Transition elements Lanthanids Actinides |
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Alkali metals |
Group 1 Extremely reactive |
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Alkaline earth metals |
Group 2 Very reactive |
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Halogen |
Group 17 Very reactive non reactive More reactive towards top |
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Noble gases |
Group 18 Not reactive |
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Representive elements |
Groups 1-2 and 13-18 Follow periodic law very closely |
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Transition elements |
Groups 3-12 Do not follow periodic law closely |
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Lanthanides |
Top row on bottom |
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Actinides |
Bottom row on bottom |
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Properties of metals |
Shiny Malleable Conducts heat and electricity |
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Aufbau principle |
Electrons enter lowest energy level |
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Paulo exclusion principle |
Electrons will pair up |
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Huds rule |
One electron per orbital until all contain 1 electron with parallel spins |
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Law of conservation of energy |
Energy is neither created not destroyed, only transformed from one form to another or transferred from one place to another. If an electron undergoes a quantum leap,energy will be released or absorbed |
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Anion |
Negative ion Gains electrons Non metals |
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Cations |
Postive ions Lose electrons .mote protons than electrons Metals |
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Types of compounds |
Molecular Ionic |
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Molecular compounds |
Non Metals Molecules |
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Ionic |
Cations and anions |
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Molecular compounds are named using |
Prefixes |
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Prefixes |
Mon - 1 Di - 2 Tri - 3 Tetra - 4 Penta - 5 Hexa - 6 Septa - 7 Octa - 8 Nona - 9 Deca - 10 |
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Covalent bond |
Share electrons |
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Ionic bond |
Transfer electrons |
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Alloy |
Two metals just mix and don't react |
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Diatomic elements |
Hydrogen Nitrogen Oxygen Fluorine Chlorine Bromine Iodine Astatine |
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Dot structure |
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Coordinate covalent bond |
When one atoms donated both electrons in a covalent bond |
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Resonance |
When more than 1 for diagram with the came connections is possible |
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Structural formula |
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Bond dissociation energy |
Energy required to break a bond . |
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Joules |
Measures of energy |
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VSEPR |
Valance Shell Electron Pair Repulsion |
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Lone pair |
Unbonded pairs |
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4 atoms bonded |
Basic shape is tetrahedral Pyramid with triangular base 109.5° |
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3 bonded and 1 lone pair |
Still basic tetrahedral Can't see electing pair Shape is original pyramidal 109.5° |
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2 bonded and 2 lone pairs |
Still tetrahedral Shape is bent 104.4° |
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3 atoms and no lone pair |
120° Shape is flat and called original planar |
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2 or 3 atoms no lone pair |
180°c shape is linear |
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Polar bonds |
When atoms in a bond are the same, the electrons are shared equally |
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Polar covalent bond |
2 different atoms are connected. The electrons may not be shared equally |
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Electronegativity |
Measure of how strongly the atoms attract electrons in a bond |
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0.0-4 |
Covalent nonpolar |
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0.4-1.0 |
Covalent moderately polar |
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1.0-2.0 |
Covalent polar |
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Greater than 2 |
Ionic |
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Intermolecular force |
What holds molecules to each other |
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Vander waals forces |
Weakest Intermolecular force |
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Dispersion |
Depends on the number of electrons in molecules |
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Diapole interaction |
Polar molecules attract |
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Accuracy |
How close a measurement is to the true value |
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Precision |
how close to the measurements are to each other |
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Accepted value |
Correct value based on reliable references |
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Experimental value |
Value measure in the lab |
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Error |
Accepted value - experimental value |
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Percent error |
Error ÷ Accepted error × 100 |
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Moles |
Amount of substance the contains 6.02×10^23 representative particles of that substance |
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Percent composition |
How much of total mass of a compound is represented by each of its elements Mass of element ÷ compound × 100 |
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Empirical formula |
Lowest while number ratio of elements in a compound |
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Molecular formula |
Actual ratio of elements in a compound |
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Types of reaction |
Combination reaction Decomposition Single replacement Double replacement |
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Combination reaction |
A+B ---> AB |
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Decomposition reaction |
AB ---> A+B |
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Single replacement reaction |
A + BC ---> B + AC |
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Double replacement reaction |
AB + CD ---> AD +CB |
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Combusion |
Makes CO2 AND H20 |
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Limiting reagent |
Limiting reagent is the reaction you run out of first |
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Actual yield |
What you get in the lab when the chemicals are mixed |
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Theoretical yield |
What the balanced equation tells you you should make |
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Percent yield |
Actual ÷ theoretical ×100 |
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If you double molecules |
Double pressure |
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More molecules |
More collisions |
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Increase temperature |
Pressure is constant |
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Kinetic molecular theory |
All matter is made up of particles that are in constant movement; chemical reactions are a resuo6 of particle collisions |
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Solute |
Dissolved particles |
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Solvent |
Dissolving medium in a solution |
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Miscible |
Describes liquids that dissolve in one another in all proportions |
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Immiscible |
Describes liquids that are insoluble in one another |
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Hydrous |
containing water as a constituent. |
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Anhydrous |
Containing no water |
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Exothermic |
process that releases heat to its surroundings |
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Ionic vs molecular |
Ionic: formula units, transfer electrons, Metals and nonmetals, high melting point,high solubility, good electrical conductor Molecules: molecules, share electrons, nonmetals, low melting point, high to low solubility, poor to no conductivity |
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Precipitate |
cause (a substance) to be deposited in solid form from a solution. |
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Multivalent |
having a valence of three or more |
